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stiv31 [10]
3 years ago
5

Cual es la temperatura de congelacion del agua

Chemistry
1 answer:
Sergio039 [100]3 years ago
7 0
<span>La temperatura de congelación del agua es 0 grados </span>centígrados. 
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Explanation:

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10.0 g of calcium carbonate was heated. The mass of calcium oxide left was 5.6 g. Calculate the mass of
Kipish [7]

Answer:

4.4g

Explanation:

Mass of CaCO3 = 10g

Mass of CaO = 5.6g

Mass of CO2 =?

Mass of CaCO3 = Mass of CaO + Mass of CO2

Mass of CO2 = Mass of CaCO3 — Mass of CaO

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3 years ago
Consider the following properties of the atmosphere of the planet Mars at a particular measurement point on the surface, as meas
Airida [17]

Answer:

a. 581.4 Pa

b. 3.33x10⁻⁴ mol/L

c. 3.49x10⁻⁴ mol/L

d. 0.015 g/L

Explanation:

a. By the Raoult's Law, the partial pressure of a component of a gas mixture is its composition multiplied by the total pressure, so:

pA = 0.9532*6.1

pA = 5.81452 mbar

pA = 5.814x10⁻³ bar

1 bar ----- 10000 Pa

5.814x10⁻³ bar--- pA

pA = 581.4 Pa

b. Considering the mixture as an ideal gas, let's assume the volume as 1,000 L, so by the ideal gas law, the total number of moles is:

PV = nRT

Where P is the pressure (610 Pa), V is the volume (1 m³), n is the number of moles, R is the gas constant (8.314 m³.Pa/mol.K), and T is the temperature.

n = PV/RT

n = (610*1)/(8.314*210)

n = 0.3494 mol

The number of moles of CO₂ is (V = 0.9532*1 = 0.9532 m³):

n = PV/RT

n = (581.4*0.9532)/(8.314*210)

n = 0.3174 mol

cA = n/V

cA = 0.3174/953.2

cA = 3.33x10⁻⁴ mol/L

c. c = ntotal/Vtotal

c = 0.3494/1000

c = 3.49x10⁻⁴ mol/L

d. The molar masses of the gases are:

CO₂: 44 g/mol

N₂: 28 g/mol

Ar: 40 g/mol

O₂: 32 g/mol

CO: 28 g/mol

The molar mass of the mixture is:

M = 0.9532*44 + 0.027*28 + 0.016*40 + 0.0008*28 = 43.36 g/mol

The mass concentration is the molar concentration multiplied by the molar mass:

3.49x10⁻⁴ mol/L * 43.36 g/mol

0.015 g/L

8 0
3 years ago
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