In a reaction Mg(s) + 2HCl(aq) → H2(g) + MgCl2(aq), 6.00 g of Mg was present at 0.00 min. After 3.00 min, 4.50 g of Mg remained. Express the average rate as gram Mg consumed/min
as with any rate of change, this would be
(4.50-6.00)/(3.00-0.00) = -1.5/3 = -0.5 g/min
since you said consumed, then that'd be just 0.5 g/min
Well, I guess you could say that the magnesium had a "mag-nificent" disappearing act in this reaction! Let's do some calculations to find the average rate of the magnesium consumption.
We have 6.00 g of magnesium at the start (0.00 min) and after 3.00 min, we're left with 4.50 g. So, the magnesium "vanished" at a rate of 1.50 g in 3.00 min.
To find the average rate per minute, we can divide the change in grams by the change in time:
Average rate = (1.50 g) / (3.00 min) = 0.50 g/min.
So, the average rate of magnesium consumption in this reaction is 0.50 g/min. The magnesium was truly a "quick change artist" in this chemical reaction!
To find the average rate of the reaction in terms of grams of Mg consumed per minute, we need to calculate the change in the amount of Mg over a given time period.
Given that 6.00 g of Mg was present initially (at 0.00 min) and after 3.00 min, 4.50 g of Mg remained, we can calculate the change in Mg.
Change in Mg = Initial Mg - Final Mg
Change in Mg = 6.00 g - 4.50 g
Change in Mg = 1.50 g
Next, we need to determine the time taken for this change to occur, which is 3.00 min.
Now, we can calculate the average rate of the reaction:
Average Rate = Change in Mg / Time
Average Rate = 1.50 g / 3.00 min
Therefore, the average rate of the reaction in terms of grams of Mg consumed per minute is 0.50 g/min.
To calculate the average rate of a reaction in terms of grams consumed per minute, we need to determine the amount of magnesium (Mg) consumed and the time interval over which it was consumed.
Given information:
- Initial amount of Mg = 6.00 g
- Final amount of Mg after 3.00 min = 4.50 g
To find the amount of Mg consumed, we subtract the final amount from the initial amount:
Amount of Mg consumed = Initial amount - Final amount
= 6.00 g - 4.50 g
= 1.50 g
The time interval over which the consumption took place is given as 3.00 minutes.
Now we can calculate the average rate of Mg consumed per minute:
Average rate = Amount of Mg consumed / Time interval
= 1.50 g / 3.00 min
= 0.50 g/min
Therefore, the average rate of Mg consumed in this reaction is 0.50 grams per minute.