Explanation:
There are many things you might do to increase your yield:
1. Limit the number of transfers. Every time you transfer a component to another container, you lose some of the compound.
2. Add more of one reactant. If your reaction is an equilibrium reaction, use a large excess of the cheapest reactant.
3. Remove a product as fast as it forms. Removal of product forces the position of equilibrium to the right and increases the yield.
4. If your reactants are gases and you have fewer moles of gaseous products, increase the pressure.
<em>The </em><em>reaction </em><em>in </em><em>which </em><em>the </em><em>heat </em><em>is </em><em>released </em><em>to </em><em>the </em><em>surrounding </em><em>is </em><em>called </em><em>exothermic </em><em>reaction</em><em>.</em>
<em>And </em><em>exothermic </em><em>reaction </em><em>can </em><em>be </em><em>identified </em><em>while </em><em>doing </em><em>chemical </em><em>reactions</em><em>.</em><em>,</em><em> </em><em>when </em><em>heat </em><em>is </em><em>released</em><em> </em><em>then </em><em>it </em><em>is </em><em>exothermic </em><em>reaction</em><em>. </em>
STP is 760. i hope this helps
Answer:
B. <u><em>At the end of the reaction, both product and reactants are of a constant concentration.</em></u>
Explanation:
- Option A and C are similar as they both refer to constant concentration of product and reactant respectively in first half. As in the graph, the concentration of reactant and product changes (concentration of reactant decreases and concentration of product increase) with time in the <em>first half</em> of the reaction. This made both A and C option wrong.
- Option D is also wrong as at the <em>end of reaction</em> the line of concentration of product and reactant do not coincide which means they are not equal.
- Option B is correct as we take the end of reaction at the point where the concentration of reactant and product won't change much or become constant
<u><em>first half</em></u> time is the when concentration of reactant reduces to 50% of initial concentration which you can nearly assume on or before the point of intersection of both the concentration graphs.
<u><em>end of reaction</em></u><em> </em>is the time when the reaction completes which is theoretically infinite but generally we take end of the reaction as the time when the slope of concentration curve becomes nearly zero or the time when change in concentration of reactant and product is negligible.
A nonmetal and a nonmetal will make molecular compounds like H2O and CO2