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3 years ago

The pressure of nitrogen gas at 35°C is changed from 0.89 atm to 4.3 atm. What will be its final temperature in Kelvin?

Chemistry

1 answer:

Alja [10]3 years ago

8 0

Answer: The final temperature in Kelvin is 1488

Explanation:

To calculate the final temperature of the system, we use the equation given by Gay-Lussac Law. This law states that pressure of the gas is directly proportional to the temperature of the gas at constant pressure.

Mathematically,

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

where,

$P_1\text{ and }T_1$ are the initial pressure and temperature of the gas.

$P_2\text{ and }T_2$ are the final pressure and temperature of the gas.

We are given:

$P_1=0.89atm\\T_1=35^0C=(35+273)K=308K\\P_2=4.3atm\\T_2=?$

Putting values in above equation, we get:

$\frac{0.89}{308}=\frac{4.3}{T_2}\\\\T_2=1488K$

Hence, the final temperature in Kelvin is 1488

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4 years ago

WHAT MASS OF WATER WILL BE PRODUCED FROM 2.70 MOLES OF CA(OH)2 REACTING WITH HCI

Keith_Richards [23]

<u>Answer:</u> The mass of water produced in the reaction is 97.2 grams

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We are given:

Moles of calcium hydroxide = 2.70 moles

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$Ca(OH)_2+HCl\rightarrow CaCl_2+2H_2O$

By Stoichiometry of the reaction:

1 mole of calcium hydroxide produces 2 moles of water

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To calculate mass for given number of moles, we use the equation:

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Molar mass of water = 18 g/mol

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Putting values in above equation, we get:

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Hence, the mass of water produced in the reaction is 97.2 grams

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4 years ago

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3 years ago

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Answer:

ou have learnt in your previous classes that the sour and bitter

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18 Science

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2.1.1 Acids and Bases in the Laboratory

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Explanation:

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