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AysviL [449]
3 years ago
5

Convert the following to grams 0.500 moles of (NH4)2CO3

Chemistry
1 answer:
steposvetlana [31]3 years ago
5 0
Molar mass (NH₄)₂CO₃ = <span>96.09 g/mol

1 mole ---------> 96.09 g
0.500 moles ----> ?

0.500 * 96.09 = 48.045 g of </span><span>(NH₄)₂CO₃

hope this helps!

</span>
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Answer:

220mol.

Explanation:

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A flask contains 6g hydrogen gas and 64 g oxygen at rtp the partial pressure of hydrogen gas in the flask of the total pressure
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Answer:

B.3/5p

Explanation:

For this question, we have to remember <u>"Dalton's Law of Partial Pressures"</u>. This law says that the pressure of the mixture would be equal to the sum of the partial pressure of each gas.

Additionally, we have a <em>proportional relationship between moles and pressure</em>. In other words, more moles indicate more pressure and vice-versa.

P_i=P_t_o_t_a_l*X_i

Where:

P_i=Partial pressure

P_t_o_t_a_l=Total pressure

X_i=mole fraction

With this in mind, we can work with the moles of each compound if we want to analyze the pressure. With the molar mass of each compound we can calculate the moles:

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6g~H_2\frac{1~mol~H_2}{2~g~H_2}=~3~mol~H_2

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The molar mass of oxygen gas (O_2) is 32 g/mol, so:

64g~H_2\frac{1~mol~H_2}{32~g~H_2}=~2~mol~O_2

Now, total moles are:

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With this value, we can write the partial pressure expression for each gas:

P_H_2=\frac{3}{5}*P_t_o_t_a_l

P_O_2=\frac{2}{5}*P_t_o_t_a_l

So, the answer would be <u>3/5P</u>.

I hope it helps!

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