Answer:
To find the volume of the gas. So if you have the amount of gas in moles. So the first step is to multiply the amount of moles that is 2.4 with liters to find the answer.
Explanation:
Answer:
Calories of candy = 5.1 kcal /g
Explanation:
Given data:
Mass of candy = 4.70 g
Change in temperature = 2.46 °C
Specific heat capacity of calorimeter = 40.50 Kj/°C
Calories present per gram = ?
Solution:
Formula
Cal of candy = specific heat capacity × change in temperature / mass
C = c . ΔT/m
C = 40.50 Kj/°C × 2.46 °C / 4.70 g
C = 99.63 kj /4.70 g
C = 21.2 kj/ g
C = 21.2 kj/ g × 0.239 kcal/kj
C = 5.1 kcal /g
The Universe
Is Not shrinking
Is Not Expanding
It Does contain billions of galaxies
And it is Not about 10 billion years old
Hope this Helps. :)
When 0.34 of HNO₃ is titrated to equivalence using 0.14 l of 0.1 m NaOH then the concentration of HNO₃ is 0.041 M
The reaction of neutralization of HNO₃ with NaOH is
HNO₃ + NaOH → H₂O + NaNo₃
When 1 mole of HNO₃ react with 1 mole of NaOH, based on chemical rection the moles of NaOH at equivalence point are equal to moles of HNO₃ present in solution: -
With the mole and volumes, we can find molarity as follows:
Moles of NaOH = moles HNO₃
⁼ 0.14 L X (0.1 mol NaOH/L) = 0.014 mole NaOH
=0.014 mol HNO₃
Molarity: -
= 0.041 M
Thus, from above solution we concluded that the concentration of HNO₃ solution is 0.041 M.
Learn more about molarity: brainly.com/question/8732513
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Answer:
Some of the calcium carbonate remained stuck to the side of the glassware after filtering
Some of the calcium carbonate spilled when measuring its mass
Explanation:
The percent yield is obtained from;
Actual yield/Theoretical yield * 100
Usually, the actual yield is less than the theoretical yield thereby making the percent yield less than 100%.
In the case of this particular reaction; when some calcium carbonate remains stuck on the glassware or some calcium carbonate is spilled during weighing, the actual yield of product obtained from the reaction becomes less than the theoretical or calculated yield hence the percent yield becomes less than 100%.
