CHEM 130 Lecture Notes - Lecture 13: Ideal Gas Law, Molar Volume, Gas Laws

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12 Mar 2015

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Chem 130: general chemistry: macroscopic investigations and reaction principles - The constant of proportionality relating the molar volume of a gas to t/p. The values of r in various units. A combination of all the gas laws. Pv = nrt, where n equals the number of moles of gas. The density of a substance is its mass divided by its volume, but because the volume of a gas varies with temperature and pressure, the density of a gas also varies with temperature and pressure.

Related Questions

The ideal gas law

PV=nRT

relates pressure P, volume V, temperature T, and number of moles of a gas, n. The gas constant R equals 0.08206 L?atm/(K?mol) or 8.3145 J/(K?mol). The equation can be rearranged as follows to solve for n:

n=PV/RT

This equation is useful when dealing with gaseous reactions because stoichiometric calculations involve mole ratios.

Part A

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

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

What is the mass of calcium carbonate needed to produce 29.0L of carbon dioxide at STP?

Part B

Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation 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 dioxide formed by the combustion of 2.00g of butane?

-Stoichiometric relationships w/ gases-

Check my solution please!

The ideal gas law : PV=nRT relates pressure P, volume V, temperature T, and number of moles of a gas, n. The gas constant R equals 0.08206 Lâ atm/(Kâ mol)or 8.3145 J/(Kâ mol). The equation can be rearranged as follows to solve for n: n=PVRT

1. When heated, calcium carbonate decomposes to yield calcium oxide and carbon dioxide gas via the reaction

CaCO3(s)âCaO(s)+CO2(g)

What is the mass of calcium carbonate needed to produce 75.0 L of carbon dioxide at STP?

2. Butane, C4H10, is a component of natural gas that is used as fuel for cigarette lighters. The balanced equation of the complete combustion of butane is 2C4H10(g)+13O2(g)â8CO2(g)+10H2O(l)

At 1.00 atm and 23 âC, what is the volume of carbon dioxide formed by the combustion of 3.80 g of butane?

CHEM 130 Lecture Notes - Lecture 13: Ideal Gas Law, Molar Volume, Gas Laws

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