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Ede4ka [16]
3 years ago
7

Liquid sodium is being considered as an engine coolant. How many grams of liquid sodium (minimum) are needed to absorb of energy

in the form of heat if the temperature of the sodium is not to increase?
Chemistry
1 answer:
umka21 [38]3 years ago
5 0

Answer:

See explanation below

Explanation:

First, you are not providing any data to solve this, so I'm gonna use some that I used a few days ago in the same question. Then, you can go and replace the data you have with the procedure here

The concentration of liquid sodium will be 8.5 MJ of energy, and I will assume that the temperature will not be increased more than 15 °C.

The expression to calculate the amount of energy is:

Q = m * cp * dT

Where: m: moles needed

cp: specific heat of the substance. The cp of liquid sodium reported is 30.8 J/ K mole

Replacing all the data in the above formula, and solving for m we have:

m = Q / cp * dT

dT is the increase of temperature. so 15 ° C is the same change for 15 K.

We also need to know that 1 MJ is 1x10^6 J,

so replacing all data:

m = 8.5 * 1x10^6 J / 30.8 J/K mole * 15 m = 18,398.27 moles

The molar mass of sodium is 22.95 g/mol so the mass is:

mass = 18,398.27 * 22.95 = 422,240.26 g or simply 422 kg rounded.

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It has been approximately 6 hours after death.

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How many moles 1 gram H2SO4
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A 35.6 g sample of ethanol (C2H5OH) is burned in a bomb calorimeter, according to the following reaction. If the temperature ros
Oksana_A [137]
<h3>Answer:</h3>

A) -1.24 × 10^3 kJ/Mol

<h3>Explanation:</h3>

we are given;

Mass of ethanol, m = 35.6 g

Temperature change, Δt(35.0 to 76.0°C) = 41 °C

Specific heat capacity of the calorimeter, c = 23.3 kJ/°C

Molar mass of ethanol = 46.07 g/mol

We are required to the heat change of the reaction.

  • We need to note that the reaction is an exothermic reaction since there is an increase in temperature which means heat was lost to the surroundings.

Therefore; we are going to use the following steps;

<h3>Step 1 : Moles of ethanol </h3>

We know, Moles = Mass ÷ molar mass

Thus, moles of ethanol = 35.6 g ÷ 46.07 g/mol

                                      = 0.773 moles

<h3>Step 2: Enthalpy change or heat change for the reaction.</h3>

Heat change = -mcΔt

but we are given s[pecific heat capacity in Kj/°C and we require heat change in kJ/mol

Therefore;

Heat change = -(cΔt) ÷ n ( n is the number of moles)

                      = -( 23.3 kJ/°C × 41°C) ÷0.773 mol

                    = - 1.24 × 10^3 kJ/Mol

Therefore, values of ΔH of the reaction is -1.24 × 10^3 kJ/Mol

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