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1. ### Hydrogen gas was collected in a gas-collecting bottle?

... of a "dry" gas..... Volume of "wet" hydrogen gas STP. Use Dalton's law of partial pressure to find the pressure of the...

1 Answers Â· Science & Mathematics Â· 04/03/2017

2. ### General Chemistry Help? How to convert ice to water assuming no heat loss?

...111111 + 92466.4] / 891,000 n = 0.79311 moles CH4 Vol. at STP .... 0.79311 X 22.4 = 17.77 L <<...

1 Answers Â· Science & Mathematics Â· 24/01/2017

3. ### Convert the following volumes to STP: A) 24.5L at 25Â°C and 104kPa B) 45.0mL at -40Â°C and 140kPa?

A) (24.5 L) x (273 K) / (25 + 273) K x (104 kPa / 101.3 kPa) = 23.0 L B) (45.0 mL) x (273 K) / (-40 + 273) K x (140 kPa / 101.3 kPa) = 72.9 mL

2 Answers Â· Science & Mathematics Â· 22/12/2016

4. ### What is the STP volume of a sample of gas which occupies 500mL at a temperature of 100Â°C and a pressure of 200kPa?

(500 mL) x (273 K) / (100 + 273) K x (200 kPa / 101.3 kPa) = 723 mL

2 Answers Â· Science & Mathematics Â· 21/12/2016

5. ### Chem MOLAR CONCENTRATION HELP?

At STP 1 mole = 22.4 L Thus, moles CO2 present = 205 L x 1 mol/22.4 L = 9.15 moles 9.15 moles /10.0 L = 0.915 moles/L = 0.915 M

1 Answers Â· Science & Mathematics Â· 29/11/2016

6. ### Hi, i have some questions in mind that i would like to answer in my essay. Thank you!?

...ligand is to fit into a G-Protein receptor in order to activate the STP. 3. Sorry, I don't know. But i answered ...

1 Answers Â· Science & Mathematics Â· 19/11/2016

7. ### Consider the following balanced equation. SiO2(s) + 4 HF(g) â†’ SiF4(s) + 2 H2O(l)?

(6.72 L HF) / (22.414 L/mol) x (1 mol SiF4 / 4 mol HF) x (104.0791 g SiF4/mol) = 7.80 g SiF4

1 Answers Â· Science & Mathematics Â· 24/10/2016

...tonne of sulphur, what is the volume of SO2 produces at STP? Obviously you have to use equation 1: S(s) + O2 (g) â†’ ...

2 Answers Â· Science & Mathematics Â· 23/08/2016

9. ### Calculate volume of co2 gas produced at STP by combustion of 20 g of methane . Ch4+2o2. Co2 +2h2?

CH4 + 2O2 ==> CO2 + 2H2O Note: your equation is incorrect. H2 gas in NOT formed. moles CH4 present: 20 g x 1 mole/16 g = 1.25 moles CH4 moles CO2 produced: 1 mole...

1 Answers Â· Science & Mathematics Â· 15/08/2016

10. ### Determine the mass and number of molecules released?

((7.94*10^1) x 10^-3 L) / (22.414 L/mol) = 0.0035424 mol NH3 (0.0035424 mol NH3) x (17.03056 g NH3/mol) = 0.0603 g NH3 (0.0035424 mol NH3) x (6.022 x 10^23 molecules/mol) = 2.13 Ă— 10^21 molecules NH3

1 Answers Â· Science & Mathematics Â· 27/07/2016