Answer:
The statement that is not true is: 'Temperature does not affect the reaction rate'.
Explanation:
a) Temperature can change a reaction rate. <u> This is true</u>
Increasing the temperature increases the reaction rates because of the disproportionately large increase in the number of high energy collisions. It is only these collisions (possessing at least the activation energy for the reaction) which result in a reaction.
For example, the time taken to melt a metal will be much higher at a lower temperature but it will decrease as soon as we increase the temperature
b) The amount of reactants can increase the reaction rate.<u> This is true</u>
A higher concentration of reactants leads to more effective collisions per unit time, which leads to an increased reaction rate.
c) Temperature can decrease the reaction rate. <u>This is true </u>
Decreasing the temperature decreases the reaction rates because of the decrease in the number of high energy collisions. It will result in a slower reaction.
d) Temperature does not affect the reaction rate. <u>This is not true. </u>
The reaction rate is temperature dependent. The reaction rate increases with higher temperature and decreases with lower temperature.
Blank 1: nothing (to keep 2 total nitrogen)
blank 2: 3 (to make 6 total hydrogen)
blank 3: 2 (to make 2 total nitrogen and 6 total hydrogen)
hope this helps!! :)
Answer:
126.0g of water were initially present
Explanation:
The electrolysis of water occurs as follows:
2H₂O(l) ⇄ 2H₂(g) + O₂(g)
<em>Where 2 moles of water produce 2 moles of hydrogen and 1 mole of oxygen.</em>
<em />
To find the mass of water we need to determine moles of oxygen and hydrogen, thus:
<em>Moles Hydrogen:</em>
14.0g H₂ ₓ (1mol / 2g H₂) = 7 moles H₂
<em>Moles Oxygen:</em>
112.0g O₂ ₓ (1mol / 32g) = 3.5 moles O₂
Based on the chemical equation, the moles of water initially present were 7 moles (That produce 7 moles H₂ and 3.5 moles O₂). The mass of 7 moles of H₂O is:
7 moles H₂O * (18g / mol) =
<h3>126.0g of water were initially present</h3>
N = 3.2 moles, T = 50 + 273 = 323 K, P = 101.325 kPa, R = 8.314 L.kPa/K.mol
PV = nRT
V = nRT / P substituting.
V = (3.2 mole)(8.314 L.kPa/K.mol )(323 K) / (<span>101.325 kPa)
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Answer:
C) to show that atoms are conserved in chemical reactions
Explanation:
When writing a chemical reaction, we should always consider the Mass Conservation Law, which basically states that; in an isolated system; the total mass should remain constant, this is, the total mass of the reactives should be equal to the total mass of the products
For this case, we should add the apporpiate coefficients in order to be in compliance with this law:
2H₂ + O₂ → 2H₂O
So, we can check the above statement:
For reactives (left side):
4H
2O
For product (right side):
4H
2O
