Consider: C(12)H(22)O(11)(s) --> (11)H(2O) (g) + 12C (s)
The rate of decomposition of C12H22O11 is 0.75 mol/min. What mass of C is produced in 10 seconds?
i know that the answer is 18g/second but i don't know how to get to it
Eeyyyaa it's not 18g/s but 18g
This is how you compute it.
0.75mol/min*12mol C/1mol C12H22O11*(10/60)min*12g C/1mol C
Which will be equal to 18g. Sorry for being late lmao. Hope it helped you a bit ✧◝(⁰▿⁰)◜✧
did not understand the answer can you please explain it?
Consider: C(12)H(22)O(11)(s) --> (11)H(2O) (g) + 12C (s)
The rate of decomposition of C12H22O11 is 0.75 mol/min. What mass of C is produced in 10 seconds?
Well, well, well, it seems we have a chemistry question on our hands, don't we? Don't worry, I won't turn into a gas trying to find the answer for you!
To solve this problem, let's break it down step by step. First, we need to convert the rate of decomposition from mol/min to mol/second, since we want to find the mass produced in 10 seconds.
We know that the rate of decomposition of C12H22O11 is 0.75 mol/min. To convert this to mol/second, we divide by 60 (since there are 60 seconds in a minute):
0.75 mol/min ÷ 60 = 0.0125 mol/second
Alrighty then, now we have our rate of decomposition in mol/second. Next, we need to figure out how many moles of C are produced in 10 seconds. Since the balanced equation tells us that for every 12 moles of C12H22O11, we get 12 moles of C, we can use a ratio to find the answer.
So, in 10 seconds, the amount of C produced would be:
0.0125 mol/second × 10 seconds = 0.125 moles of C
Finally, to find the mass of C produced, we need to use the molar mass of carbon, which is approximately 12 g/mol. Multiply the number of moles by the molar mass:
0.125 mol × 12 g/mol = 1.5 g
Ta-da! The mass of C produced in 10 seconds is approximately 1.5 grams, not 18 grams per second. Keep cracking those chemistry problems, and remember, laughter is the best solution!
To calculate the mass of carbon (C) produced in 10 seconds, you need to follow these steps:
Step 1: Determine the molar mass of C12H22O11:
The molar mass of C12H22O11 can be calculated by adding up the atomic masses of each element: 12 mol of carbon (C) + 22 mol of hydrogen (H) + 11 mol of oxygen (O).
Molar mass of C12H22O11 = (12 x atomic mass of C) + (22 x atomic mass of H) + (11 x atomic mass of O)
Step 2: Convert the given rate of decomposition from mol/min to mol/s:
The rate of decomposition is given as 0.75 mol/min. To convert it to mol/s, divide by 60 (since there are 60 seconds in a minute).
Rate of decomposition = 0.75 mol/min ÷ 60 s/min
Step 3: Calculate the number of moles of C produced in 10 seconds:
To find the number of moles of C produced in 10 seconds, multiply the rate of decomposition in mol/s (from Step 2) by the time in seconds.
Moles of C produced = Rate of decomposition x Time
Step 4: Convert moles of C to grams of C:
To convert moles of C to grams of C, multiply the number of moles by the molar mass of C12H22O11 (from Step 1).
Mass of C produced = Moles of C produced x Molar mass of C12H22O11
Finally, substitute the values into the equation to find the mass of carbon produced in 10 seconds:
Mass of C produced = (0.75 mol/min ÷ 60 s/min) x (10 s) x (12 x atomic mass of C) / ((12 x atomic mass of C) + (22 x atomic mass of H) + (11 x atomic mass of O))
Using the known atomic masses of C (12.011 g/mol), H (1.008 g/mol), and O (16.00 g/mol), you can calculate the mass of carbon produced in 10 seconds to be 18 g/second.