a)What is the ratio of hydrogen atoms (H) to oxygen atoms (O) in 2 L of water? Enter the simplest whole-number ratio in the order of hydrogen to oxygen, respectively. Express your answer as two integers, separated by a comma (e.g., 3,4). b) How many atoms of hydrogen (H) are present in 200 molecules of ammonia (NH3)?Express your answer numerically. c) Magnesium oxide decomposes into magnesium and oxygen. If 4.03g of magnesium oxide decomposes to form 2.43g of magnesium, what mass of oxygen gas is also released in the reaction? Express the mass of oxygen numerically in grams.

Chemistry

answer

watching

217

views

coralrabbit151Lv1

11 Dec 2019

a)What is the ratio of hydrogen atoms (H) to oxygen atoms (O) in 2 L of water? Enter the simplest whole-number ratio in the order of hydrogen to oxygen, respectively. Express your answer as two integers, separated by a comma (e.g., 3,4).

b) How many atoms of hydrogen (H) are present in 200 molecules of ammonia (NH₃)?
Express your answer numerically.

c) Magnesium oxide decomposes into magnesium and oxygen. If 4.03g of magnesium oxide decomposes to form 2.43g of magnesium, what mass of oxygen gas is also released in the reaction?

Express the mass of oxygen numerically in grams.

answer

watching

217

views

For unlimited access to Homework Help, a Homework+ subscription is required.

You have 0 free answers left.
Get unlimited access to 3.8 million step-by-step answers.

Get unlimited access

Already have an account? Log in

Kenneth DuqueLv10

13 Oct 2020

Unlock all answers

Get 1 free homework help answer.

Already have an account? Log in

Join us on Discord

Chemistry Study Group

Join now

Related questions

Please answer the questions 13-16 marked as the âREPORT FOR EXPERIMENT 3â by reading the first 4 pictures if it helps.

EXPERIMENT 3 Preparation and Properties of Oxygen MATERIALS AND EQUIPMENT Solids: candles, magnesium (Mg) strips, dry yeast, fine steel wool (Fe), wood splints. Solution: 3 percent hydrogen peroxide (HOp), pneumatic trough, 20 to 25 em length rubber tubing, 25 X 200 mm ignition tube, five wide-mouth (gas-collecting) bottles, five glass cover plates. DISCUSSION Oxygen is the most abundant and widespread of all the elements in the earth's crust. It occurs both as free oxygen gas and combined in compounds with other elements. Free oxygen gas is diatomic and has the formula O2 Oxygen is found combined with more elements than any other single element, and it will combine with all the elements except some of the noble gases. Water is 88.9 percent oxygen by mass and the atmosphere is about 21 percent oxygen by vol- ume. Oxygen gas is colorless and odorless, and is only very slightly soluble in water, a prop- erty important to its collection in this experiment. Oxygen may be obtained by decomposing a variety of oxygen-containing compoun of these are mercury(ID oxide (HgO, mercuric oxide), leadIV) oxide (PbO2, lead dioxide), potas- sium chlorate (KCIO,), potassium nitrate (KNO,), hydrogen peroxide (H02), and water (H,O). In this experiment oxygen is produced by decomposing hydrogen peroxide, and five bottles of oxygen will be collected by the downward displacement of water. After collection, some the physical and chemical properties of oxygen will be observed. A. Decomposition of Hydrogen Peroxide to Generate Oxygen Hydrogen peroxide decomposes very slowly at room temperature. The rate of decomposition is greatly increased by adding a catalyst, manganese dioxide. Although manganese dioxide contains oxygen, it is not decomposed under conditions of this experiment. These equations represent the changes that occur Word Equation: Hydrogen peroxide Water + Oxygen Formula Equation: 2H,0,la)H,oN)+ 0g) B. Collection of Oxygen The oxygen is collected by a method known as the downward displacement of water. The gas is conducted from a generator to a bottle of water inverted in a pneumatic trough

An empty 5.00-L flask is charged with 0.250 g of pure H2S(g), at 25 âC.

In addition to the H2S already present in the flask, solid NH4HS is added until there is excess unreacted solid remaining.

Part C

What are the partial pressures of NH3 and H2S at equilibrium, that is, what are the values of PNH3and PH2S, respectively?

Enter the partial pressure of ammonia followed by the partial pressure of hydrogen sulfide numerically in atmospheres separated by a comma

PNH3, PH2S =

Part D

What is the mole fraction, Ï, of H2S in the gas mixture at equilibrium?

Express your answer numerically.

Part E

What is the minimum mass of NH4HS that must be added to the 5.00-L flask when charged with the 0.250 g of pure H2S(g), at 25 âC to achieve equilibrium?

Express your answer numerically in grams.

Ammonium bisulfide, NH4HS , forms ammonia, NH3 , and hydrogen sulfide, H2S , through the reaction NH4HS(s)âNH3(g)+H2S(g) This reaction has a Kp value of 0.120 at 25 âC .

An empty 5.00-L flask is charged with 0.300 g of pure H2S(g) , at 25 âC .

--------------------------------------------------------------------------------------------

PART A

What are the partial pressures of NH3 and H2S at equilibrium, that is, what are the values of PNH3 and PH2S , respectively?

Enter the partial pressure of ammonia followed by the partial pressure of hydrogen sulfide numerically in atmospheres separated by a comma.

PNH3 , PH2S = _____ atm

------------------------------------------------------------------------------------------

PART B

What is the mole fraction, Ï , of H2S in the gas mixture at equilibrium?

Express your answer numerically.

ÏH2S = ?

-------------------------------------------------------------------------------------------

PART C

What is the minimum mass of NH4HS that must be added to the 5.00-L flask when charged with the 0.300 g of pure H2S(g) , at 25 âC to achieve equilibrium?

mass>

_________ g ??