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4 years ago

Which law relates to the ideal gas law?

Chemistry

2 answers:

professor190 [17]4 years ago

8 0

Answer: The law that related the ideal gas law is $\frac{V_1}{n_1}=\frac{V_2}{n_2}$

Explanation:

There are 4 laws of gases:

Boyle's Law: This law states that pressure is inversely proportional to the volume of the gas at constant temperature.

Mathematically,

$P_1V_1=P_2V_2$

Charles' Law: This law states that volume of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$

Gay-Lussac Law: This law states that pressure of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

$\frac{P_1}{T_1}=\frac{P_2}{T_2}$

Avogadro's Law: This law states that volume is directly proportional to number of moles at constant temperature and pressure.

Mathematically,

$\frac{V_1}{n_1}=\frac{V_2}{n_2}$

Hence, the law that related the ideal gas law is $\frac{V_1}{n_1}=\frac{V_2}{n_2}$

e-lub [12.9K]4 years ago

8 0

Answer:

c on edge 2020

Explanation:

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What volume will a balloon occupy at 1.0 atm, if the balloon has a volume of 7.6 l at 3.8 atm?

sergejj [24]

From the Boyle's law, it is clear that volume is inversely proportional to pressure. Thus it is prudent to say that, P1V1=P2V2
From the question above,
P1=1atm
P2=3.8atm
V1=?
V2=7.6L
Hence, 1*V1=3.8atm*7.6L
V1=28.88L

4 0

3 years ago

Read 2 more answers

What volume of 1.25 M solution is needed to make 250 mL of 0.75 M solution?

zysi [14]

Answer:

V1= 150ml

Explanation:

C1= 1.25, V1=?, C2= 0.75, V2= 250ml

Applying dilution formula

C1V1= C2V2

V1= (0.75×250)/1.25 = 150ml

6 0

3 years ago

Based on this reaction, find how many moles of co can be obtained starting with 7 mol ch4?

Klio2033 [76]

I will solve the question assuming the reaction used as below
1 CH4(g) + 1 H2O(g) ==> 1 CO(g) + 3 H2(g)

In the reaction, CH4 is the reactant and CO is the wanted product. If you look at the coefficient of the substance, for every 1 mol of CH4 react there will be 1 mol of CO produced. So, if you have 7 moles of CH4 the amount of CO produced would be: 7 moles * 1/1= 7 moles of CO

5 0

4 years ago

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The reaction for the formation of phosgene from carbon monoxide and chlorineCO + Cl2 --> COCl2 is first order in CO and secon

Ilya [14]

Answer:

$r = k . [CO] .[Cl_{2}]$

Explanation:

Let´s consider the following reaction:

CO + Cl₂ ⇒ COCl₂

The general rate law is:

$r = k . [CO]^{m}. [Cl_{2}]^{n}$

where,

r is the rate of the reaction

k is the rate constant

[CO] and [Cl₂] are the molar concentrations of each reactant

m and n are the reaction orders for each reactant

Since the reaction is first order in CO, m = 1. The overall order is the sum of all the individual orders. In this case, the overall order m + n = 2. Then,

m + n = 2

n = 2 - m = 2 - 1 = 1

The reaction is first order in Cl₂.

The rate law is:

$r = k . [CO]. [Cl_{2}]$

6 0

4 years ago

What would the temperature of 0.734 moles of chlorine gas be at 1.83 atmospheres in a 10.2

lesya [120]

Answer: 310K

Explanation:

Given that:

Volume of Chlorine gas V = 10.2L

Temperature T = ?

Pressure P = 1.83 atm

Number of moles of chlorine gas N = 0.734 moles

Molar gas constant R is a constant with a value of 0.0821 atm L K-1 mol-1

Then, apply ideal gas equation

pV = nRT

1.83atm x 10.2L= 0.734 moles x 0.0821 atm L K-1 mol-1 x T

18.67atm L = 0.0603 atm L K-1 x T

T = (18.67atm L / 0.0603 atm L K-1)

T = 309.8K (Round up to 310K)

Thus, the temperature of the chlorine gas is 310 kelvin

5 0

4 years ago