Answer:
47.8 moles of H₂O.
Explanation:
We'll begin by writing the balanced equation for the reaction. This is illustrated below:
2H₂ + O₂ —> 2H₂O
From the balanced equation above,
1 mole of O₂ reacted to produce 2 moles of H₂O
Finally, we shall determine the number of mole of water, H₂O, produced by the reaction of 23.9 moles of O₂. This can be obtained as follow:
From the balanced equation above,
1 mole of O₂ reacted to produce 2 moles of H₂O.
Therefore, 23.9 moles of O₂ will react to produce = 23.9 × 2 = 47.8 moles of H₂O.
Thus, 47.8 moles of H₂O were obtained from the reaction.
The food has 23629.64 cal
<h3>Further explanation</h3>
Given
mass = 1000 g of water
temperature increases 23.65 * C
Required
The energy of the food
Solution
Heat absorbed by water :
Q = m . c . Δt
Q = 1000 g x 4.184 J/g°C x 23.65 °C
Q = 98951.6 J
1 Joules = 0.2388 Calories
98951.6 J = 23629.64 cal
Answer:
ga
Explanation:
beacuse it its the voltage that high
Answer:
The correct answer is 16.8 g (option C)
Explanation:
Step 1: Data given
9.78 grams + 7.0 grams
Rule significant numbers say:
⇒ Non-zero digits are always significant.
⇒ Any zeros between two significant digits are significant.
⇒ A final zero or trailing zeros in the decimal portion ONLY are significant.
For addition and subtraction, look at the places to the decimal point. Add or subtract in the normal way, then round the answer to the LEAST number of places to the decimal point of any number in the problem.
9.78 g+ 7.0 g = 16.78 grams
Significant numbers = 1 decimal
16.78 ⇒ 16.8
The correct answer is 16.8 g (option C)
