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3 years ago

CH4(g) + 2O2(g) = CO2(g) + 2H2O(g)

Chemistry

1 answer:

krek1111 [17]3 years ago

3 0

Answer:

0.04 moles of CH₄ are required

Explanation:

Given data:

Number of moles of CH₄ required = ?

Number of moles of O₂ present = 0.08 mol

Solution:

Chemical equation:

CH₄ + 2O₂ → CO₂ + 2H₂O

now we will compare the moles of oxygen and methane.

O₂ : CH₄

2 : 1

0.08 : 1/2×0.08 = 0.04

Thus, 0.04 moles of CH₄ are required.

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The gas law for an ideal gas at absolute temperature T (in kelvins), pressure P (in atmospheres), and volume V (in liters) is PV

allsm [11]

Answer:

The rate of change of the temperature is 0.0365 Kelvin per minute.

Explanation:

Step 1: Given data

ideal gas law: P*V = n*R*T

with P= pressure of the gas ( in atm) = 9.0 atm

with V= volume of the gass (in L) =12L

with n = number of moles = 10 moles

R = gas constant = 0.0821 L*atm* K^−1*mo^−1

T = temperature = TO BE DETERMINED

The volume decreases with a rate of 0.17L/min = dV/dT = -0.17

The pressure increases at a rate of 0.13atm/min = dP/dT

Step 2: The ideal gas law

P * [dV/dT] + V * [dP/dT] = nR * dT/dt

9 atm * (-0.17L/min) + 12L * 0.13atm/min = 10 moles * 0.0821 L*atm* K^−1*mo^−1 *dT/dt

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dT/dt = 0.03/0.821

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