(3b-301-4.12) Carborundum is silicon carbide, SiC, a very hard material used as an abrasive on sandpaper and in other applications. It is prepared by the reaction of pure sand, SiO2, with carbon at high temperature. Carbon monoxide, CO, is the other product of this reaction. The balanced equation is shown below. How many grams of the carbon monoxide side product are produced from 4.12 moles of SiO2? Show all work and round your answer to three significant figures. SiO2 + 3C → SIC + 2CO

(3b-301-4.12) Carborundum is silicon carbide, SiC, a very hard material used as an abrasive on sandpaper and in other applications. It is prepared by the reaction of pure sand, SiO2, with carbon at high temperature. Carbon monoxide, CO, is the other product of this reaction. The balanced equation is shown below. How many grams of the carbon monoxide side product are produced from 4.12 moles of SiO2? Show all work and round your answer to three significant figures. SiO2 + 3C → SIC + 2CO

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Kaolinite, a clay mineral with the formula Al4Si4O10(OH)8, is produced naturally by the chemical weathering of aluminum silicate minerals like feldspar (granite). Kaolinite is used industrially as filler in slick-paper for magazines and as a raw material for ceramics. How many grams of oxygen are present in 14.79 g of kaolinite?
The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen. P4 + 5O2 ⟶ P4O10 Calculate the percent yield if 2.6 g of P4 reacts with 23.3 g of O2 to yield 4.6 g of P4O10 from the reaction.
In preparation of ammonia (NH3), the reaction of 7.2 g of H2 with 75 g of N2 produced 36 g of ammonia. What is the percentage yield of this reaction? N2 + H2 - NH3 44% 66% 132% 88% 97%
Balance the following chemical equation (if necessary): C5H10(g)O2(g) -> H2O(g)+CO2(g)
Determine the theoretical yield In grams of Li3N that can be formed from 3.53 g of ? Assume an excess of nitrogen Hint: Calculate the molar mass of and . 6 () + N29) > 2 (s) 2. Calculate the percent yield the actual yield is 3.55 g O2
2. If 2.500 g of Na2CO3 is used in the reaction, calculate the theoretical yield of NaCl.
What is the theoretical yield of SO3SO3 produced by 2.02 gg of SS? Express your answer numerically in grams.
According to the balanced chemical question below, how many grams of K 3N can be formed from 0.61 moles of K? Assume an excess of nitrogen gas. The molar mass of potassium nitride (K 3N) is 131.30 g/mol.6 K (s) + N 2 (g) ? 2K 3N (s) A 0.392 g B 26.7 g C 160. g D 4.42 g E 37.5 g
Cryolite, Na, AlF,(s), an ore used in the production of aluminum, can be synthesized using aluminum oxide. Balance the equation for the synthesis of cryolite. equation: Al,0,(s) + NaOH(1) + HF(g) → Na, AIF, + H,O(g) 6. If 13.4 kg of Al,0,(s), 56.4 kg of NaOH(1), and 56.4 kg of HF(g) react completely, how many kilograms of cryolite will be produced? mass of cryolite produced: kg Na, AIF, Which reactants will be in excess? HF NaOH Question Source: McQuarrie, Rock, And Gallogly 4e - General Chemsitry Publisher: University Science Books S A étv Aa MacBook Air 80 000 000 DII DD F3 F4 F5 F6 F7 F8 F9 F10 F11 F12
Sodium hydroxide reacts with phosphoric acid to yield sodium phosphate and water. If 45 g of NaOH reacts with 35 g of H3PO4, what is the limiting reagent of this reaction if it yields a certain amount of NA3PO4? (Atomic masses: Na = 22.99 u ; O = 16.00 u; H = 1.01 u ; P = 30.97 u) Phosphoric Acid Sodium Hydroxide Water Sodium Phosphate 00
Carborundum is silicon carbide, SiC. It is prepared by the reaction of pure sand, SiO2 with carbon at high temperature. CO is the other product of this reaction. Given the equation SiO2 + 3C results in 2CO + SiC calculate how much SiO2 is required to produce 3.00 kg of SiC.
Chlorine dioxide, ClO2, is used for bleaching paper. It is also the gas used to kill the anthrax spores that contaminated the US Hart Senate building in 2001. Chlorine dioxide is prepared by treating sodium chlorite, NaClO2, with chlorine gas. What is the mass of chlorine dioxide that can be prepared from 5.50 kg of sodium chlorite? Balanced Equation: 2NaClO2 + Cl2 -----> 2ClO2 + 2 NaCl hello can u write the solution I cannot understand if written in words :(