Answer: D. Converting energy stored in chemical bonds into electricity.
Explanation:
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Answer:
We assume you are converting between moles CCl4 and gram. You can view more details on each measurement unit: molecular weight of CCl4 or grams This compound is also known as Carbon Tetrachloride. The SI base unit for amount of substance is the mole. 1 mole is equal to 1 moles CCl4, or 153.8227 grams.
Explanation:
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Answer:
Explanation:
2 HCl(g) + Mg(s) → MgCl₂(s) + H₂(g)
Let's calculate the quantity of mole of produced hydrogen with the Ideal Gases Law
P . V = n . R .T
2.19 atm . 6.82L = n . 0.082 . 308K
(2.19 atm . 6.82L) / (0.082 . 308K) = n
0.591 mol = n
1 mol of H₂ gas came from 2 mol of hydrochloric, so, 0.591 mol came from the double of mole
0.591 .2 = 1.182 mole of acid.
Molar mass of HCl = 36.45 g/m
1.182 mole are (36.45 g/m . 1.182g ) contained in 43.1 g
Density HCl = HCl mass / HCl volume
0,118 g/mL = 43.1 g / HCl volume
43.1 g / 0.118 g/mL = 365.3 mL (HCl volume)
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Looking at the information given in the description, the experiment is testing for the effects of the different salts on the growth of the plants.
This means that the type of salt is the independent variable, or the variable being manipulated and tested.
To ensure fair results, some parts of the experiment would need to be kept the same, which is the control. The only answer choice that makes sense in this instance is A. water.
THE KINETIC MOLECULAR THEORY STATES THAT ALL PARTICLES OF AN IDEAL GAS ARE IN CONSTANT MOTION AND EXHIBITS PERFECT ELASTIC COLLISIONS.
Explanation:
An ideal gas is an imaginary gas whose behavior perfectly fits all the assumptions of the kinetic-molecular theory. In reality, gases are not ideal, but are very close to being so under most everyday conditions.
The kinetic-molecular theory as it applies to gases has five basic assumptions.
- Gases consist of very large numbers of tiny spherical particles that are far apart from one another compared to their size.
- Gas particles are in constant rapid motion in random directions.
- Collisions between gas particles and between particles and the container walls are elastic collisions.
- The average kinetic energy of gas particles is dependent upon the temperature of the gas.
- There are no forces of attraction or repulsion between gas particles.
