assuming you mean 30gs-3 this means 30 grams per thousandth of a second
3^6 = 729
27 3 to the power of 3 3 x 3 x 3 (3 x 3) x 3 9 x 3 27
2 x 3 x 3 x 3 = 54 2 x 3 x 5 x 7 = 210 2 x 3 x 3 x 3 x 5 x 7 = 1890, the LCM
2 x 2 x 2 x 3 x 3 x 3 = 216 2 x 2 x 2 x 2 x 2 x 3 x 3 = 288 2 x 2 x 2 x 3 x 3 x 5 = 360
2 x 2 x 2 x 2 x 3 x 3 x 3 x 3 x 5 = 6480
20 x 500 mg = 10g or 10g = 500mg x 20
10g/410g X 100 = 2.4 2.5 %
I had to do this problem on a sample exam I got from the University of South Carolina. It has to do with a stoichiometry reaction. If I got the answer wrong, I apologize but this is how I did it. I'll use 2 approaches so you can understand all the concepts going into it. And forget about the "excess H_2" so it doesn't throw you off. First write a balanced equation of the reactants and product: N_2 + 3H_2 -----> 2NH_3 N_2 = 10g 10g of N_2 x [1 mol N_2 / (14.0067x2)] x (3 mol H_2 / 1 mol N_2) x [(1.0079x2) / 1 mol H_2] so, 10 x (1 / 28.0134) x (3) x (2.0158), is 10 x (.03569) x (3) x (2.0158) = 2.158 grams of H_2 Since we have 10g of N_2, we can add the two numbers and find out the mass of ammonia. 10g + 2.158 = 12.158g, or 12 g NH_3. Similarly we can substitute the ammonia (NH_3) for the H_2 in the equation above and get the same answer. 10g of N_2 x [1 mol N_2 / (14.0067x2)] x (2 mol NH_3 / 1 mol N_2) x [(14.0067 + (1.0079 x 3)) / 1 mol NH_3] so, 10 x (1 / 28.0134) x (2) x (17.0304), is 10 x (.03569) x (2) x (17.0304) = 12.158 g, or 12 g NH_3
If you are on 10g or later and the recycle bin feature is turned on, you can use the FLASHBACK TABLE x TO BEFORE DROP command, where x is the name of the table. If it is not there, or the recycle bin feature is not available, you will have to restore the table from a backup.
5(X - 5) + 2g(X - 5)-------------------------------all the factoring I can see
To determine the number of atoms in 10g of Fe, you first need to calculate the number of moles of Fe using its molar mass (55.85 g/mol). Then, you can use Avogadro's number (6.022 x 10^23 atoms/mol) to find the number of atoms in those moles of Fe. Finally, multiply the number of moles by Avogadro's number to get the total number of atoms in 10g of Fe.
1 kg = 1000g (kilo=1000)0.01 kg = 0.01 x 1000g = 10g
10G networks transfer at a maximum of 10 gigabits per second.
To calculate the number of moles in 10g of iodine, you need to first determine the molar mass of iodine (I), which is 126.9 g/mol. Then, you can use the formula: moles = mass / molar mass. So, moles = 10g / 126.9 g/mol ≈ 0.079 moles of iodine.
After 2 half-lives (two half-lives of tritium is 12.32 x 2 = 24.64 years), the initial 10g sample of tritium would have decayed by half to 5g.
No, they do NOT contain the same number of particles (either molecules N2 or atoms C): there molecular or atomic mass is different.Look at this:10g N2 / 28 (g/mole N2) x 6.022x1023 (molecules N2/mole N2) = 2.15 x1023 molecules N210g C / 12 (g/mole C) x 6.022x1023 (atoms C/mole C) = 5.02 x1023 atoms C
10 grams nitrogen (1 mole N/14.01 grams)(6.022 X 1023/1 mole N) = 4.3 X 1023 atoms of nitrogen ======================