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wel
4 years ago
11

2.5 piece of lithium is dropped into a 500 g sample of water at 22.1 C.ten temperature of the water increases to 23.5 C. How muc

h heat energy is released in the reaction
Chemistry
1 answer:
Dominik [7]4 years ago
3 0

Answer:

2.6 kJ  

Explanation:

The formula for the amount of heat (q) absorbed by the water is

q = mCΔT

1. Calculate ΔT

ΔT = 23.5 °C - 22.1 °C = 1.4 °C

2. Calculate q

q₂ = mCΔT = 500 g × 4.184 J·°C⁻¹g⁻¹ × 1.4 °C = 2900 J = 2.9 kJ

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5 hours and 25 minutes
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3 years ago
Consider the following reaction: AB(s)⇌A(g)+B(g) . At equilibrium, a 10.9 L container at 650 K contains A(g) at a pressure of 0.
irina1246 [14]

Answer:

pA = 0.095 atm

pB = 0.303 atm

Explanation:

Step 1: the reaction

AB(s) ⇔ A(g) + B(g)

Kp = pA * pB

⇒ with Kp = equilibrium constant

Kp = 0.126 * 0.23  ⇒ Kp = 0.02898

Since the container will be compressed to half of its original volume, means that he pressure will be doubled.

⇒pA = 0.252

⇒pB =0.46

To establish this equilibrium, each pressure has to be lowered by x

⇒pA = 0.252 - x

⇒pB = 0.46 - x

Kp = 0.02898 = (0.252 - x)(0.46-x)

0.02898 = 0.11592 - 0.252x -0.46x + x²

-x² + 0.712x - 0.08694 = 0

D= b² - 4ac

⇒ D = 0.712² -4*(-1) *(-0.08694) = 0.506944‬ -0.34776‬ =0.159184

x = (-b ± √D)/2a  

x = (-0.712 ± √0.159184)/(2*-1)  = (-0.712 ± 0.398978696)/-2

x = 0.156510652 or x= 0.555489348

x = 0.555489348 is impossble or the pressure would be negative

x=0.156510652

pA =0.252 - 0.156510652 = 0.095489348 atm

pB = 0.46 - 0.156510652 = 0.303489348 atm

4 0
3 years ago
2C4H10+13O2-->8CO2+10H2O Using the predicted and balanced equation, How many Liters of CO2 can be produced from 150 grams of
Anna11 [10]

Answer:  233 L of CO_2 will be produced from 150 grams of  C_4H_{10}

Explanation:

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}  \text{Moles of} C_4H_{10}=\frac{150g}{58g/mol}=2.59moles

The balanced chemical equation is:

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

According to stoichiometry :

2 moles of C_4H_{10} produce =  8 moles of CO_2

Thus 2.59 moles of C_4H_{10} will produce=\frac{8}{2}\times 2.59=10.4moles  of CO_2  

Volume of CO_2=moles\times {\text {Molar volume}}=10.4moles\times 22.4mol/L=233L

Thus 233 L of CO_2 will be produced from 150 grams of  C_4H_{10}

8 0
3 years ago
Combustion analysis of 63.8 mg of a c, h and o containing compound produced 145.0 mg of co2 and 59.38 mg of h2o. what is the emp
Makovka662 [10]
<span>: The empirical formula for the compound is C3H60 (see below) CO2 is the only product containing C, C produced = 145.0 mg CO2 x (1 g / 1000 mg) x (1 mole CO2 / 44.0 g CO2) x (1 mole C / 1 mole CO2) = 0.00330 moles C. H2O is the only product containing H, H produced = 59.38 mg H2O x (1 g / 1000 mg) x (1 mole H2O / 18.0 g H2O) x (2 moles H / 1 mole H2O) = 0.00660 moles H. Oxygen is in both and the unknown reacts with oxygen(in the air) 0.00330 moles C x (12.0 g C / 1 mole C) = 0.0396 g C = 39.6 mg C 0.00660 moles H x (1.01 g H / 1 mole H) = 0.00667 g H = 6.7 mg H Because the unknown weighed 63.8 mg and consists off justC, H, and O, then mass O = g unknown - g C - g H = 63.8 mg - 39.6 mg - 6.7 mg = 17.5 mg = 0.0175 g 0.0175 g O x (1 mole O / 16.0 g O) = 0.00109 moles O The mole ratio of C:H:O is: C = 0.00330 H = 0.00660 O = 0.00109 Divide by the smallest you get: C = 0.00330 / 0.00109 = 3.03 H = 0.00660 / 0.00109 = 6.06 O = 0.00109 / 0.00109 = 1.00</span>
6 0
4 years ago
3) What is the molarity of a solution that has 27.6 g of propanol (C3H2O) dissolved in 325 mL of solution? The molar mass of eth
Novosadov [1.4K]

Answer:

Explanation:

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7 0
3 years ago
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