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2 years ago

What is the volume of 10.5 moles of nitrogen gas at STP

2 answers:

5 0

The volume of 10.5 moles of nitrogen gas at STP (Standard Temperature and Pressure) is 235.339 liter of gas. This problem can be solved by using the PV=nRT or V= nRT/V equation which is the relation between the molar volume, the temperature, and the pressure of gas. In this formula, P is the pressure (1 atm @STP), R is the universal gas constant ( 0.0821 atm L/mol K), n is the molecule amount (10.5), V is the molecular volume, and T is the temperature ( 273 K @STP).

The calculation for the problem above: 10.5*0.0821*273/1 = 235.339

Jobisdone [24]2 years ago

3 0

The volume of 10.5 moles of nitrogen at standard temperature and pressure (STP) would be 235.33 L. Calculating this value, we assume that the gas is ideal so we use the equation PV = nRT. At STP, temperature is 273.15 K and pressure is 1 atm. We calculate as follows:

V = nRT / P
V = 10.5 (0.08205)(273.15) / 1
V = 235.33 L

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2 years ago

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2 years ago

Formic acid, which is a component of insect venom, has a ka = 1.8 ´ 10-4. what is the [h3o+] in a solution that is initially 0.1

scoray [572]

Answer is: concentratio of H₃O⁺ ions is 4.2·10⁻³ M.
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2 years ago

At 500 K the reaction 2 NO(g) + Cl2(g) ⇌ 2 NOCl(g) has Kp = 51 In an equilibrium mixture at 500 K, the partial pressure of NO is

Aleks [24]

Answer:

p3=0.36atm (partial pressure of NOCl)

Explanation:

2 NO(g) + Cl2(g) ⇌ 2 NOCl(g) Kp = 51

lets assume the partial pressure of NO,Cl2 , and NOCl at eequilibrium are P1 , P2,and P3 respectively

$Kp=\frac{[NOCl]^{2} }{[NO]^{2} [Cl_2] }$

$Kp=\frac{[p3]^{2} }{[p1]^{2} [p2] }$

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p3=?

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On solving;

p3=0.36atm (partial pressure of NOCl)

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2 years ago