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Mkey [24]
2 years ago
14

A 390 mL solutions of 4.6 M HCl is left out over the weekend and 74 mL of solvent evaporates. What is the new concentration of H

Cl?
Chemistry
1 answer:
storchak [24]2 years ago
8 0

Answer:

5.7 M

Explanation:

You have .390 L of 4.6 M HCl.

.390 L * 4.6 mol/L = 1.794 mol HCl

.390-.074=.316 L solvent remaining

1.794 mol/.316 L=5.7 M HCl

You might be interested in
If 250 g of calcium chlorate decomposes into calcium chloride and oxygen what mass of oxygen would be produced
andrey2020 [161]

Answer:

m O2 = 116,16 g

Explanation:

Ca(ClO3)2 ------------> CaCl2 + 3O2

n Ca(ClO3)2 = 250/207 = 1,21 mol

n O2 = 3n Ca(ClO3)2 = 1,21 * 3 = 3,63 mol

m O2 = 3,63 * 32 = 116,16 g

4 0
3 years ago
What happens in a neutralization reaction?
mina [271]

Answer:

Answer is letter B

Explanation:

The first one is wrong because acids release H+, not bases.

The third one is wrong because the pH is exactly 7, not greater.

The last one is wrong because it is vague and does not fit a neutralization reaction.

7 0
2 years ago
Butane C4H10 (g),(Hf = –125.7), combusts in the presence of oxygen to form CO2 (g) (Delta.Hf = –393.5 kJ/mol), and H2O(g) (Delta
shusha [124]

Answer: The enthalpy of combustion, per mole, of butane is -2657.4 kJ

Explanation:

The balanced chemical reaction is,

2C_4H_{10}(g)+13O_2(g)\rightarrow 8CO_2(g)+10H_2O(g)

The expression for enthalpy change is,

\Delta H=[n\times H_f_{products}]-[n\times H_f_{reactants}]

Putting the values we get :

\Delta H=[8\times H_f_{CO_2}+10\times H_f_{H_2O}]-[2\times H_f_{C_4H_{10}+13\times H_f_{O_2}}]

\Delta H=[(8\times -393.5)+(10\times -241.82)]-[(2\times -125.7)+(13\times 0)]

\Delta H=-5314.8kJ

2 moles of butane releases heat = 5314.8 kJ

1 mole of butane release heat = \frac{5314.8}{2}\times 1=2657.4kJ

Thus enthalpy of combustion per mole of butane is -2657.4 kJ

3 0
3 years ago
How many grams of XeF6 are required to react with 0.579 L of hydrogen gas at 6.46 atm and 45°C in the reaction shown below?
ankoles [38]
The chemical reaction equation for this is 

XeF6 + 3H2 ---> Xe + 6HF

Assuming gas behaves ideally, we use the ideal gas formula to solve for number of moles H2 with T = 318.15K (45C), P = 6.46 atm, V = 0.579L. Then we use the gas constant R = 0.08206 L atm K-1 mol-1.

we get n = 0.1433 moles H2

to get the mass of XeF6, 

we divide 0.1433 moles H2 by 3 since 1 mole XeF6 needs 3 moles H2 to react then multiply by the molecular weight of XeF6 which is 245.28 g/mole XeF6.

0.1433 moles H2 x \frac{1 mole XeF6}{3 moles H2} x \frac{245.28 g XeF6}{1 mole XeF6} = 11.71 g XeF6

Therefore, 11.71 g of XeF6 is needed to completely react with 0.579 L of Hydrogen gas at 45 degrees Celcius and 6.46 atm.
3 0
3 years ago
Q05 the "atomic number" of an atom is determined by the number of ________ it has.
Alexxx [7]
The atomic number of an atom is determined by the number of protons it has..

It is also the whole number shown on the periodic table 
6 0
3 years ago
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