For the following reaction what would happen if you did the following. Would it speed up or slow down?
Mg + HCl → MgCl2 + H2 + heat
• Adding heat
• Grinding up the magnesium
• Lowering the concentration of HCl
• Burning the hydrogen gas as soon as it is produced
• Dipping the reaction into ice water.
Mg + HCl → MgCl2 + H2 + heat
• Adding heat
• Grinding up the magnesium
• Lowering the concentration of HCl
• Burning the hydrogen gas as soon as it is produced
• Dipping the reaction into ice water.
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1. Adding heat would slow down this reaction, since heat is a product.
2. Grinding up the magnesium would speed up the reaction, since more surface area would be exposed to the HCl, allowing molecular collisions to occur at a faster rate.
3. Lowering the concentration of HCl would slow down the reaction, because molecular collisions would occur more slowly.
4. Burning the Hydrogen gas would speed up the rate of reaction.
5. Dipping it in ice water would reduce heat, speeding up the reaction.
Take-home lessons: Rate of reaction increases as you increase concentration of reactants or decrease concentration of products. Rate of reaction decreases as you decrease concentration of reactants or increase concentration of products.
2. Grinding up the magnesium would speed up the reaction, since more surface area would be exposed to the HCl, allowing molecular collisions to occur at a faster rate.
3. Lowering the concentration of HCl would slow down the reaction, because molecular collisions would occur more slowly.
4. Burning the Hydrogen gas would speed up the rate of reaction.
5. Dipping it in ice water would reduce heat, speeding up the reaction.
Take-home lessons: Rate of reaction increases as you increase concentration of reactants or decrease concentration of products. Rate of reaction decreases as you decrease concentration of reactants or increase concentration of products.