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3 years ago

How much heat is absorbed when 4.5g of ice at 0°C melts to water at 10°C?

Chemistry

1 answer:

atroni [7]3 years ago

5 0

Answer: 90.45 joules

Explanation:

The quantity of Heat Energy (Q) absorbed by ice depends on its Mass (M), specific heat capacity (C) and change in temperature (Φ)

Thus, Q = MCΦ

In this case,

Q = ?

Mass of ice = 4.5g

C = 2.010 J/g°C (Though not provided, but the specific heat capacity of ice is 2.010 J/g°C)

Φ = (Final temperature - Initial temperature)

= 10°C - 0°C = 10°C

Then, Q = MCΦ

Q = 4.5g x 2.010 J/g°C x 10°C

Q = 90.45 joules

Thus, 90.45 joules of heat is absorbed by ice.

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2 years ago

Gaseous ammonia chemically reacts with oxygen O2 gas to produce nitrogen monoxide gas and water vapor. Calculate the moles of ox

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Answer : The number of moles of oxygen needed are, 1.5 moles.

Explanation :

The balanced chemical reaction will be:

$4NH_3+5O_2\rightarrow 4NO+6H_2O$

Now we have to calculate the moles of oxygen.

From the balanced chemical reaction we conclude that,

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Therefore, the number of moles of oxygen needed are, 1.5 moles.

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3 years ago

The expression of the theoretical yield (TY) in function of limiting reagent (LR) of a reaction is as follows: TY = ideal mole r

spin [16.1K]

Answer: The theoretical yield of acetanilide is 6.5 grams.

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For aniline:

Given mass of aniline = $4.50\times 10^0=4.50g$ (We know that: $10^0=1$ )

Molar mass of aniline = 93.13 g/mol

Putting values in equation 1, we get:

$\text{Moles of aniline}=\frac{4.50g}{93.13g/mol}=0.048mol$

For acetic anhydride:

To calculate the mass of acetic anhydride, we use the equation:

$\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}$

Volume of acetic anhydride = $(1.25\times \text{Mass of aniline})=1.25\times 4.50=5.625mL$

Density of acetic anhydride = 1.08 g/mL

Putting values in above equation:

$1.08g/mL=\frac{\text{Mass of acetic anhydride}}{5.625mL}\\\\\text{Mass of acetic anhydride}=(1.08g/mL\times 5.625mL)=6.08g$

Given mass of acetic anhydride = 6.08 g

Molar mass of acetic anhydride = 102.1 g/mol

Putting values in equation 1, we get:

$\text{Moles of acetic anhydride}=\frac{6.08g}{102.1g/mol}=0.06mol$

The chemical equation for the reaction of aniline and acetic anhydride follows:

$C_6H_5NH_2+CH_3COOCOCH_3\rightarrow C_6H_5NHCOCH_3+CH_3COOH$

By Stoichiometry of the reaction:

1 mole of aniline reacts with 1 mole of acetic anhydride

So, 0.048 moles of aniline will react with = $\frac{1}{1}\times 0.048=0.048mol$ of acetic anhydride

As, given amount of acetic anhydride is more than the required amount. So, it is considered as an excess reagent.

Thus, aniline is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

1 mole of aniline produces 1 mole of acetanilide

So, 0.048 moles of aniline will produce = $\frac{1}{1}\times 0.048=0.048mol$ of acetanilide

Now, calculating the theoretical yield of acetanilide by using equation 1:

Moles of acetanilide = 0.048 moles

Molar mass of acetanilide = 135.17 g/mol

Putting values in equation 1, we get:

$0.048mol=\frac{\text{Mass of acetanilide}}{135.17g/mol}\\\\\text{Mass of acetanilide}=(0.048mol\times 135.17g/mol)=6.5g$

Hence, the theoretical yield of acetanilide is 6.5 grams.

3 0

3 years ago

a thermometer containing 8.3g of mercury has broken. if mercury ha a density of 13.6g/mL. what volume is spilled?

scoray [572]

D = m / V

13.6 = 8.3 / V

V = 8.3 / 13.6

V = 0.610 mL

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4 0

3 years ago

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