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seraphim [82]
2 years ago
10

What type of energy warms earths surface?

Chemistry
1 answer:
Scrat [10]2 years ago
8 0
A. solar energy

the earth is warmed by the sun, which is solar (or infrared).
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Using tongs place the 250 mL beaker on hot plate
LenKa [72]

Answer:

just use the tongs and put it on a plate

Explanation:

4 0
2 years ago
Which two values for `DeltaG` and E°cell correctly indicate a spontaneous reaction?
Mila [183]

Well as an spontaneous reaction will have a negative gibbs free energy (delta g) and a positive e cell and also the E cell is also measured in V, then your answer is the first one: ΔG = –295kJ, E°cell = +1.53 v. Hope this works



4 0
3 years ago
The complete combustion of copper(I) sulphide is according to the following equation:
MaRussiya [10]

Answer:

a) 7.94 x 10²³ molecules, b) 5.62 g SO2, c) 1.97 L

Explanation:

a) We need to first convert Cu2S to moles. Since molar mass of Cu2S is 159.14 g/mol, 14.0 g = 0.0880 mol. Using molar ratios (3 mol O2/2 mol Cu2S, 0.0880 mol of Cu2S = 0.132 mol O2. Since 1 mol contains 6.02 x 10²³ molecules, 0.132 mol O2 = 7.94 x 10²² molecules O2.

b) Since the molar ratios of Cu2S to SO2 is 1:1, 0.0880 mol of Cu2S produces 0.0880 mol SO2. To convert mol to grams, we use the molar mass of SO2 (64.06 g/mol) to figure out that 0.0880 mol SO2 = 5.63 g SO2.

c) At STP, 1 mol occupies 22.4 liters. 0.0880 mol SO2 x 22.4 L/1 mol = 1.97 L

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5 0
3 years ago
Tetrahydrofuran (THF) is a common organic solvent with a boiling point of 339 K. Calculate the total energy (q) required to conv
poizon [28]

Explanation:

For the given reaction, the temperature of liquid will rise from 298 K to 339 K. Hence, heat energy required will be calculated as follows.

             Q_{1} = mC_{1} \Delta T_{1}

Putting the given values into the above equation as follows.

           Q_{1} = mC_{1} \Delta T_{1}

                      = 27.3 g \times 1.70 J/g K \times 41

                      = 1902.81 J

Now, conversion of liquid to vapor at the boiling point (339 K) is calculated as follows.

           Q_{2} = energy required = mL_{v}

    L_{v} = latent heat of vaporization

Therefor, calculate the value of energy required as follows.

             Q_{2} = mL_{v}

                         = 27.3 \times 444

                         = 12121.2 J

Therefore, rise in temperature of vapor from 339 K to 373 K is calculated as follows.

            Q_{3} = mC_{2} \Delta T_{2}

Value of C_{2} = 1.06 J/g,    \Delta T_{2} = (373 -339) K = 34 K

Hence, putting the given values into the above formula as follows.

             Q_{3} = mC_{2} \Delta T_{2}

                       = 27.3 g \times 1.06 J/g \times 34 K

                       = 983.892 J

Therefore, net heat required will be calculated as follows.

            Q = Q_{1} + Q_{2} + Q_{3}

                = 1902.81 J + 12121.2 J + 983.892 J

                = 15007.902 J

Thus, we can conclude that total energy (q) required to convert 27.3 g of THF at 298 K to a vapor at 373 K is 15007.902 J.

5 0
3 years ago
2. How many grams of N2 are required to produce 10.0 grams of NH3? N2 + 3 H2 - 2 NH3
SOVA2 [1]

8.24g

Explanation:

Given parameters;

Mass of NH₃ = 10g

Unknown:

Mass of N₂ = ?

Solution:

  Reaction equation:

               N₂    +    3H₂     →      2NH₃

Step 1: Convert 10.0 g of NH₃ into moles of NH₃

number of moles = \frac{mass}{molar mass}

   molar mass of NH₃ = 14 + 3(1) = 17g/mol

 Number of moles = \frac{10}{17}  = 0.59mole

Step 2: Convert the moles of NH₃ calculated in Step 1 into moles of N₂

       1 mole of N₂    produced 2 mole of NH₃

   

0.59 moles of ammonia would be formed by \frac{0.59}{2} mole = 0.29mole of N₂

Step 3: Convert the moles of N₂ calculated in Step 2 into grams of N₂.

Mass of N₂ = number of moles x molar mass

  Molar mass of N₂ = 14 x 2 = 28g/mol

  Mass of N₂ = 0.29 x 28 = 8.24g

learn more:

Number of moles brainly.com/question/1841136

#learnwithBrainly

6 0
3 years ago
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