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2 years ago

How many moles of CaC2 are needed to react completely with 45.0g H2O?

Chemistry

1 answer:

sertanlavr [38]2 years ago

6 0

Answer:

In order to react with 45 g of water 1.25 moles of CaC₂ are required.

Explanation:

Given data:

Moles of CaC₂ needed = ?

Mass of water = 45.0 g

Solution:

Chemical equation:

CaC₂ + 2H₂O → C₂H₂ + Ca(OH)₂

Number of moles of water:

Number of moles = mass/ molar mass

Number of moles = 45 g/ 18 g/mol

Number of moles = 2.5 mol

Now we will compare the moles of water and CaC₂ from balance chemical equation:

H₂O : CaC₂

2 : 1

2.5 : 1/2×2.5 =1.25 mol

In order to react with 45 g of water 1.25 moles of CaC₂ are required.

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2 years ago

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2 years ago

At 1.01 bar, how many moles of CO2 are released by raising the temperature of 1 litre of water from 20∘C to 25∘C

Tatiana [17]

Answer: 0.0007 moles of $CO_2$ is released when temperature is raised.

Explanation:

To calculate the number of moles, we use the ideal gas equation, which is:

$PV=nRT$

where,

P = pressure of the gas = 1.01 bar

V = Volume of the gas = 1L

R = Gas constant = $0.08314\text{ L bar }mol^{-1}K^{-1}$

Number of moles when T = 20° C

Temperature of the gas = 20° C = (273 + 20)K = 293K

Putting values in above equation, we get:

$1.01bar\times 1L=n_1\times 0.0814\text{ L bar }mol^{-1}K^{-1}\times 293K\\n_1=0.04146moles$

Number of moles when T = 25° C

Temperature of the gas = 25° C = (273 + 25)K = 298K

Putting values in above equation, we get:

$1.01bar\times 1L=n_2\times 0.0814\text{ L bar }mol^{-1}K^{-1}\times 298K\\n_2=0.04076moles$

Number of moles released = $n_1-n_2=0.04146-0.04076=0.0007moles$

Hence, 0.0007 moles of $CO_2$ is released when temperature is raised from 20° C to 25° C

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2 years ago