sagarsunuwar8

When 5.00 mL of a sodium nitrite solution containing 17.04 g/L of sodium nitrite is added to 25.00 mL of sulfamic acid solution containing 2.754 g/L of sulfamic acid, the following reaction occurs:

HSO3NH2 (aq) + NaNO2 (aq) --> N2(g) + NaHSO4 (aq) + H2O (l)

a) Determie the mass of nitrogen gas produced, and calculate the volume occupied by this mass of gas at a temperature of 23 degrees C and a pressure of 00.5 kPa

b) When this experiment was carried out by a student and the nitrogen gas was collected over water, the volume of “wet” nitrogen produced (at 23°C and 99.5 kPa) was 14.81 mL. What was the percentage yield obtained by the student? The vapour pressure of water at 23°C is 2.81 kPa.

what acadamic discipiline are used to study information system and how does each contribute to anunderstandingof information system

Ammonium nitrite decomposes to give off nitrogen gas and liquid water. How many grams of ammonium nitrite must have reacted if 2.58 L of gas was collected over water in a gas collecting tube at 21.0°C and 97.8 kPa?

Balanced equation:

Will the volume of nitrogen (from the previous problem) INCREASE, DECREASE or remain the SAME if... *Explain briefly*

...the experiment is done at significantly higher temperature?

B. ...the amount of ammonium nitrite was increased?

C.

...the experiment was not collected over water?

Phosphorus and chlorine react as follows: P4(s) + Cl2(g) => PCl3(l). Balance it! Assume 135 g P4(s) react with 333 g of Cl2(g).

a) What is the limiting reactant?

b) What is the reactant in excess and the amount in excess?

c) What mass of phosphorus trichloride can be formed from the reaction?

What is the mass of excess reactant (in grams) that remains after the limiting reagent produces the maximum amount of phosphorus pentachloride possible upon the reaction of 4.98 g of phosphorus with 14.31 g of chlorine according to the following reaction:

P_{4 (s)} + 10 Cl_{2 (g)} → 4 PCl_{5 (l)}

Give your answer to 2 decimal places.

____Units____

1.Calculate the number of moles of PCl5 that can be produced from30.0 of P4 (and excess Cl2 ).
2.Calculate the number of moles of PCl5 that can be produced from53.0 of Cl2 (and excess P4 ).
Then, compare the two values. The reactant that produces thesmaller amount of product is the limiting reactant

According to the unbalanced chemical equation below, when 13.5 moles of phosphorus react with 40.0 moles of chlorine, what is the limiting reactant and how much excess reactant is left?

P₄ + Cl₂ ---> PCl₅

Explain these answers

Describe what you understand by the phrase "investing in your education."

900.0 mL of 3.00M phosphoric acid, H PO, reacts with 235 grams of iron (III) carbonate.

Balanced Equation: Fez(CO;) + 2H;PO4 - 2FePO4 + 3H20 + 3C02

a. Determine the limiting reactant. Show all work!

Two eneterprising students decide to develop an alternative to alka-seltzer tablet, replacing the aspirin ( acetylsaylicylic acid) with vitamin C ( ascrobic acid). One tablet would contain the following:Ingredient Formula Quantity (mg) sodium bicarbonate NaHCO3 1991 citric acid H3C6H5O7 886 vitamin C HC6H7O6 370 inert binder 1753 Total Mass 5000 a. A student dissolves a tablet of alka seltzer in water , it "fizzes" as the bicarbonate reacts with the citric acid and the vitamin C. What mass (in milligrams) of NaHCO3 reacts with the vitamin C? b. What mass (in milligrams) of NaHCO3 reacts with the citric acid? c. What mass ( in milligrams) of CO2 is released during this reaction? d. The remaining NaHCO3 is avaialble to neutralize stomach acid. What mass ( in milligrams) of stomach HCL could be neutralized by one tablet?

The first step in the reaction of Alka-Seltzer with stomach acid consists of one mole of sodium bicarbonate (NaHCO3) reacting with one mole of hydrochloric acid (HCl) to produce one mole of carbonic acid (H2CO3), and one mole of sodium chloride (NaCl). Using this chemical stoichiometry, determine the number of moles of carbonic acid that can be produced from 2 mol of NaHCO3 and 7 mol of HCl.

1)If 4.09 moles of C5H12 reacts with excess O2, how many moles of CO2 will be produced in the following combustion reaction?

2)The first step in the reaction of Alka-Seltzer with stomach acid consists of one mole of sodium bicarbonate (NaHCO3) reacting with one mole of hydrochloric acid (HCl) to produce one mole of carbonic acid (H2CO3), and one mole of sodium chloride (NaCl).

Using this chemical stoichiometry, determine the number of moles of carbonic acid that can be produced from 5 mol of NaHCO3 and 8 mol of HCl.

How much excess reactant remains after the reaction?

Using the equation NaHCO3 + HCl ---> NaCl + H20 + CO2, how many milliliters of carbon dioxide (at STP) are produced when 3.00 mL of 1.0 M hydrochloric acid reacts with excess sodium bicarbonate?

How many milliters of carbon dioxide gas can be produced at 78°C at 45.5 psi pressure with 900.0 mL of 3.00M phosphoric acid and 235 grams of iron (III) carbonate?