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2 years ago

What is the volume of a solution that has a molarity of 0.600M and contains 4.50 grams of NH4OH?

Chemistry

1 answer:

wariber [46]2 years ago

7 0

Answer:

The volume is 214, 3 ml

Explanation:

We calculate the weight of 1 mol of NH4OH:

Weight 1 mol NH4OH= Weight N + (Weight H) * 5 + Weight 0

Weight 1 mol NH4OH= 14g + 1 g* 5 + 16g = 35 g/mol

1 mol NH4OH-----35 g

0,6mol NH4OH----X=(0,6mol NH4OHx 35 g)/1 mol NH4OH= 21 g

We have 0,6 mol in 1000ml of solution (0,600 M)

21g NH4OH-----------1000ml

4,50 g NH4OH------x= (4,50 g NH4OH x 1000ml)/21 g NH4OH= 214, 2857143 ml

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3 years ago

Salt is dissolved in a flask of tap water. Distilling the mixture causes the salt to separate from the water. Which type of ener

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2 years ago

Read 2 more answers

A scientist measures the standard enthalpy change for the following reaction to be -17.2 kJ : Ca(OH)2(aq) 2 HCl(aq)CaCl2(s)

elixir [45]

Answer: $\Delta H^{0}=-173.72$ kJ/mol

Explanation: Enthalpy Change is the amount of energy in a reaction - absorption or release - at a constant pressure. So, Standard Enthalpy of Formation is how much energy is necessary to form a substance.

The standard enthalpy of formation of HCl is calculated as:

$\Delta ^{0}=\Sigma H_{products}-\Sigma H_{reactants}$

$Ca(OH)_{2}_{(aq)}+2HCl_{(aq)}$ → $CaCl_{2}_{(s)}+2H_{2}O_{(l)}$

Standard Enthalpy of formation for the other compounds are:

Calcium Hydroxide: $\Delta H^{0}=$ -1002.82 kJ/mol

Calcium chloride: $\Delta H^{0}=$ -795.8 kJ/mol

Water: $\Delta H^{0}=$ -285.83 kJ/mol

Enthalpy is given per mol, which means we have to multiply by the mols in the balanced equation.

Calculating:

$-17.2=[-795.8+2(285.85)]-[-1002.82+2\Delta H]$

$-17.2=-1367.46+1002.82-2\Delta H$

$2\Delta H=17.2-364.64$

$\Delta H=-173.72$

So, the standard enthalpy of formation of HCl is -173.72 kJ/mol

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2 years ago

Find the actual yield when the theatrical yield is 1.09g and percent yield is 90%.

ioda

Actual yield/Theoretical yield *100= Percentage yield. So Actual yield = Percentage yield*Theoretical yield.
Therefore actual yield= 90/100 * 1.09g = 0.98g

Actual yield: 0.98 g

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2 years ago