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choli [55]
3 years ago
15

3.75 g of an unknown gas at 59 °C and 1.00 atm is stored in a 1.35-L flask. What is the molar mass of the gas?

Chemistry
1 answer:
MAXImum [283]3 years ago
4 0
You need to find moles of the gas, so you would use the ideal gas law:
PV=nRT
Pressure
Volume
n=moles
R= gas constant
Tenperature in Kelvin
n= PV/RT
(1.00atm)(1.35L)/(.08206)(332K) = 0.050mol
Molar mass is grams per mole, so
(3.75g/.050mol) = 75g/mol
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Which one of the following will change the value of an equilibrium constant?
Ad libitum [116K]

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(E) changing temperature

Explanation:

Consider the following reversible balanced reaction:

aA+bB⇋cC+dD

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- The reaction must be balanced with the written coefficients as the minimum possible integer value in order to obtain the correct value of Kc

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