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larisa86 [58]
3 years ago
12

Question 15 need this answered asap (chemistry)

Chemistry
1 answer:
Tcecarenko [31]3 years ago
8 0

Answer:

80.7 L

Explanation:

PV = nRT

P = 1520 mmHg = 2 atm

n = 5 mol

R = 0.08206 (L * atm)/(mol * K)

T = 393.15 K

2 (V) = 5 (0.08206) (393.15)

V ≈ 80.7 L

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2 years ago
What is the molar mass of 37.96 g of gas exerting a pressure of 3.29 on the walls of a 4.60 L container at 375 K?
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The molar mass of the gas is 77.20 gm/mole.

Explanation:

The data given is:

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Using the ideal Gas Law will give the number of moles of the gas. The formula is

PV= nRT    (where R = Universal Gas Constant 0.08206 L.atm/ K mole

Also number of moles is not given so applying the formula

n= mass ÷ molar mass of one mole of the gas.

n = m ÷ x   ( x  molar mass) ( m mass given)

Now putting the values in Ideal Gas Law equation

PV = m ÷ x RT

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15.134 = 1168.1241  ÷ x

15.134x = 1168.1241

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If all the units in the formula are put will get cancel only grams/mole will be there. Molecular weight is given by gm/mole.

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3 years ago
Increasing the temperature, as noted in the graph, increases the rate of this chemical reaction. What is the relationship betwee
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8 0
3 years ago
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