siddharthshukla7754

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Let S be the subspace of ?4 consisting of the solutions to the following system of equations

1. Given 8.88 mL of 2.00M NaOH, calculate the number of grams of NaOH in the solution. (MW NaOH 39.99 g/mol)

2. Given 3.98 mL of sulfuric acid (98.0%) calculate the number of mmols in the solution.
(MW H₂SO₄: 98.08 g/mol, density: 1.840 g/mL)

3. Given 7.04 g of HBr calculate the volume (mL) of a 48.0% solution.
(MW HBr: 80.91 g/mol, density: 1.49 g/mL)

How many grams of solute are present in the following solutions?

A) 575mL of a 2.00M solution of nitric acid, HNO3 (MW: 63.0128g/mol)

B) 1.65L of a 0.286M solution of alanine, C3H7NO2 (MW: 89.0932g/mol)

Find the pH for the following:

A 7.98 x 10-2 M solution of HNO, (nitric acid).

If p > 5 is prime, and p is divided by 10 (that is, p = 10q + r, with 0 ≤ r < 10), show that the only possible remainders are r = 1,3,7,9.

1- When heated, calcium carbonate decomposes to yield calcium oxideand carbon dioxide gas via the reaction

CaCO3(s)?CaO(s)+CO2(g)

2- Butane,

C4H10,is a component of natural gas that is used as fuel for cigarettelighters. The balanced equation of the complete combustion ofbutane is

2C4H10(g)+13O2(g)?8CO2(g)+10H2O(l)

At 1.00 atmand 23 ?C,what is the volume of carbon dioxide formed by the combustion of1.00gof butane?

When heated, calcium carbonate decomposes to yield calcium oxideand carbon dioxide gas via the reaction

CaCO3(s)?CaO(s)+CO2(g)

What is the mass of calcium carbonate needed to produce 71.0L ofcarbon dioxide at STP? and Butane, C4H10, is a component of naturalgas that is used as fuel for cigarette lighters. The balancedequation of the complete combustion of butane is

2C4H10(g)+13O2(g)?8CO2(g)+10H2O(l)

At 1.00 atm and 23 ?C, what is the volume of carbon dioxideformed by the combustion of 2.00g of butane?

Part A) When heated, calcium carbonatedecomposes to yield calcium oxide and carbon dioxide gas via thereaction:
CaCO3(s) -> CaO(s)+CO2(g)

How many grams of calcium carbonate are needed to produce 47.0 L ofcarbon dioxide at STP?

Part B) Butane, C4H10, is a component of naturalgas that is used as fuel for cigarette lighters. The balancedequation of the complete combustion of butane is:
2C4H10(g)+13O2(g) -> 8CO2(g)+ 10H2O(l)

At 1.00atm and 23degrees C, how many liters of carbon dioxide areformed by the combustion of 1.00 g of butane?

Using the equation:2C4H10+13O2——> 8CO2+10H2O

If you produce 11.2g of water,how many liters of carbon dioxide are produced at 9.3 atm and 300*K?