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3 years ago

Help. The answer to question 1 I didn't mean to click so please answer that as well.

Chemistry

1 answer:

Zepler [3.9K]3 years ago

4 0

We have that energy=specific heat * change in temperature * mass. Thus, we have the final temperature (22) minus the initial temperature (55) to equal -33 as our change in temperature. Our specific heat is in J/g*C, so we're good with that because g stands for grams and the aluminium is measured in grams. As there are 10 grams of aluminum, we have
$10*(-33)*0.902=-298 ish$ as our final temperature

An exothermic reaction would release energy and would therefore lose heat itself, while an endothermic reaction would absorb energy and gain heat. Therefore, losing heat would be an exothermic reaction

Feel free to ask further questions!

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HELP PLZ

Vinvika [58]

Answer:

1). 19.9

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3 years ago

6. A. If 4.50 mols of ethane, C2H6, undergoes combustion according to the unbalanced equation

uranmaximum [27]

Answer:

for one mole of C2H6 there are 7/2 mole of O2 required. so for4. 50 moles you require 4.50 x 7/2 = 15.75 moles of O2.

Explanation:

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3 years ago

The northern lights and huge power surges in technology are both effects of what

umka2103 [35]

Solar winds. Plasma particles from the sun affect earth's atmosphere and cause magnetic interferance.

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3 years ago

3. A 4.00 gram sample of solid gold was heated from 274K to 314K. How much energy was involved?

MrMuchimi

Q = mcΔT = (4.00 g)(0.129 J/g•°C)(40.85 °C - 0.85 °C)
Q = 20.6 J of energy was involved (more specifically, 20.6 J of heat energy was absorbed from the surroundings by the sample of solid gold).

3 0

2 years ago

Urea, CH4N2O (s), is manufactured from NH3 (g) and CO2 (g). H2O (l) is another product of this reaction. An experiment is starte

Katarina [22]

Answer:

a. 4.41 g of Urea

b. 1.5 g of Urea

Explanation:

To start the problem, we define the reaction:

2NH₃ (g) + CO₂ (g) → CH₄N₂O (s) + H₂O(l)

We only have mass of ammonia, so we assume the carbon dioxide is in excess and ammonia is the limiting reactant:

2.6 g . 1mol / 17g = 0.153 moles of ammonia

Ratio is 2:1. 2 moles of ammonia can produce 1 mol of urea

0.153 moles ammonia may produce, the half of moles

0153 /2 = 0.076 moles of urea

To state the theoretical yield we convert moles to mass:

0.076 mol . 58 g/mol = 4.41 g

That's the 100 % yield reaction

If the percent yield, was 34%:

4.41 g . 0.34 = 1.50 g of urea were produced.

Formula is (Yield produced / Theoretical yield) . 100 → Percent yield

3 0

3 years ago