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Daniel [21]
3 years ago
6

A Solute is the part of the mixture that is A. dissolved B.used to dissolve a substance

Chemistry
1 answer:
8_murik_8 [283]3 years ago
5 0
It is the thing being dissolved!!
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If 50. 75 g of a gas occupies 10. 0 l at stp, 129. 3 g of the gas will occupy ________ l at stp.
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22.4L

of any gas contains 1 mol of that gas.

50.75g/10L*22.4L/1 mol= 113.68g/mol- this is the mole weight of your gas

1 mol/113.68g*129.3g=1.137403 mol

Set up a ratio

1.137403mol/x L=1 mol/22.4 L

X=25.477827L, or with sig figs, x=25.5L

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3 years ago
Reactants are substances that?
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A mixture of 0.10 mol of NO, 0.050 mol of H2, and 0.10 mol of H2O is placed in a 1.0- L vessel at 300 K . The following equilibr
umka2103 [35]

Answer:

The concentration of N2 at the equilibrium will be 0.019 M

Explanation:

Step 1: Data given

Number of moles of NO = 0.10 mol

Number of moles of H2 = 0.050 mol

Number of moles of H2O = 0.10 mol

Volume = 1.0 L

Temperature = 300K

At equilibrium [NO]=0.062M

Step 2: The balanced equation

2NO(g) + 2H2(g) → N2(g) + 2H2O(g)

Step 3: Calculate the initial concentration

Concentration = Moles / volume

[NO] = 0.10 mol / 1L = 0.10 M

[H2] = 0.050 mol / 1L = 0.050 M

[H2O] = 0.10 mol / 1L = 0.10 M

[N2] = 0 M

Step 4: Calculate the concentration at the equilibrium

[NO] at the equilibrium is 0.062 M

This means there reacted 0.038 mol (0.038M) of NO

For 2 moles NO we need 2 moles of H2 to produce 1 mol N2 and 2 moles of H2O

This means there will also react 0.038 mol of H2

The concentration at the equilibrium is 0.050 - 0.038 = 0.012 M

There will be porduced 0.038 moles of H2O, this means the final concentration pf H2O at the equilibrium is 0.100 + 0.038 = 0.138 M

There will be produced 0.038/2 = 0.019 moles of N2

The concentration of N2 at the equilibrium will be 0.019 M

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