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How do I calculate moles of a reactant? Final temperature C (maximum) Initial temperature C (minimum) Temperature change (T) Reaction 1: 37.91°C, 23.78°C, 26.089°C Reaction 2: 23.0°C, 11.8°C, 0.8°C Reaction 3: 36.03°C, 24.93°C, 11.1°C Q=mcΔT Q=mCAT m=1033 C=4.185/9 T=118 m=1039 C=4.183/g/c 4T=O8 =.1-13b/81201=001 L hbb'8LLh n=m/Mm eoHboinbsooH1TJURUOYniU S notbss 36 aio smdmoo owowo2 no1oHi 3. Calculate the enthalpy change, H, for each reaction in terms of kJ/mol of each reactant. H= 1000 SHOW ALL CALCULATIONS Reaction 1 qsystom(J) 5080J Number of moles Reaction 2 Reaction 3 -4779J -344.4J H(kJ/mole Questions

          How do I calculate moles of a reactant?
Final temperature C (maximum) Initial temperature C (minimum) Temperature change (T)
Reaction 1: 37.91°C, 23.78°C, 26.089°C
Reaction 2: 23.0°C, 11.8°C, 0.8°C
Reaction 3: 36.03°C, 24.93°C, 11.1°C
Q=mcΔT
Q=mCAT m=1033 C=4.185/9 T=118 m=1039 C=4.183/g/c 4T=O8
=.1-13b/81201=001 L hbb'8LLh
n=m/Mm eoHboinbsooH1TJURUOYniU S notbss 36 aio smdmoo owowo2 no1oHi
3. Calculate the enthalpy change, H, for each reaction in terms of kJ/mol of each reactant. H= 1000
SHOW ALL CALCULATIONS Reaction 1 qsystom(J) 5080J Number of moles
Reaction 2
Reaction 3 -4779J
-344.4J
H(kJ/mole
Questions

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how do i calculate moles of a reactant final temperature c maximum initial temperature c minimum temperature change t reaction 1 3791c 2378c 26089c reaction 2 230c 118c 08c reaction 3 3603c 43137

Added by Alvaro S.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Jennifer Hudspeth

09/17/2021

Step 1

Step 1: Calculate the heat absorbed or released in each reaction using the formula Q = mcΔT, where Q is the heat absorbed or released, m is the mass of the reactant, C is the specific heat capacity, and ΔT is the temperature change. Show more…

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How do I calculate moles of a reactant? Final temperature C (maximum) Initial temperature C (minimum) Temperature change (T) Reaction 1: 37.91°C, 23.78°C, 26.089°C Reaction 2: 23.0°C, 11.8°C, 0.8°C Reaction 3: 36.03°C, 24.93°C, 11.1°C Q=mcΔT Q=mCAT m=1033 C=4.185/9 T=118 m=1039 C=4.183/g/c 4T=O8 =.1-13b/81201=001 L hbb'8LLh n=m/Mm eoHboinbsooH1TJURUOYniU S notbss 36 aio smdmoo owowo2 no1oHi 3. Calculate the enthalpy change, H, for each reaction in terms of kJ/mol of each reactant. H= 1000 SHOW ALL CALCULATIONS Reaction 1 qsystom(J) 5080J Number of moles Reaction 2 Reaction 3 -4779J -344.4J H(kJ/mole Questions

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00:01 Hi there.

00:02 This problem is a conversion problem, so we will set it up using dimensional analysis.

00:08 To use dimensional analysis, we need some equalities.

00:12 So picking some of the qualities of the problem, we see that 136 kilojoules of energy are released per mole of reactant.

00:25 So one mole of the reactant will give us 136 kilojoules of energy.

00:34 We also see that it takes 4 .67 joules of energy to raise the temperature of the water 1 degrees celsius.

00:47 So for every degree celsius is 4 .67 joules.

00:52 And i see jewels and kilojoules here.

00:54 So i have a feeling i am going to need to be able to convert between joules and kilojoules.

01:02 Just like with any metric unit, the prefix kilo means 1 ,000.

01:06 So 1 ,000 joules.

01:08 Equals one kilojoule.

01:10 All right, let's see if we can set this up to produce the answer of the number of moles.

01:17 So we're trying to get from the temperature change, which is 10 .2 degrees celsius to the number of moles of reactant.

01:26 All right, so first of all, i am going to use this middle equality here and set it up as a conversion factor.

01:38 For every 1 degrees celsius, it's 4 .67 joules of energy required...

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