Enter the formula of the missing substance (Y) in the balanced equation below. Do not give the coefficient. Mg + 2HCI -- MgCl2 + Y BALANCING CHEMICAL EQUATIONS INT-T03/S02 Enter the formula of the missing substance (Y) in the balanced equation below. Do not give the coefficient. 16Y + Sg8K2S FORMING EQUATIONS INT-T01/S03 Enter an unbalanced chemical equation that summarizes this statement: the reaction of solid silicon and solid octasulfur produces solid silicon disulfide.

Balance the chemical equation. CS₂ + NH3 H₂S + NH4SCN Assume the coefficient of NHSCN is 1. What is the balanced equation? CS₂ + NH3→H₂S+NHSCN

A small fire breaks out at the accident scene. You notice that the source is a compound with the formula CgH6. You also know that the combustion reaction requires O2 and produced carbon dioxide and water. Choose the correctly balanced reaction for CgH6. C8H6+1908CO₂ + 3H₂O 2C8H6+ 1902 16CO2 + 6H₂O C8H6+19/2 02 → 8CO2 + 3H₂O C8H6+902 8CO₂ + 3H₂O

For the following unbalanced chemical equation, suppose that exactly 2.00 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of H2O is expected (assuming that the limiting reactant is completely consumed). H2 (g) + MnO2 (s) → Mn0(s) + H2 O(1) Limiting reactant: Mass of H20 = For each of the following unbalanced chemical equations, suppose that exactly 1.90 g of each reactant is taken. Determine which reactant is limiting, and calculate what mass of ICI is expected (assuming that the limiting reactant is completely consumed). I2 (s) + Cl2 (9) → ICI(9) Limiting reactant: Mass of ICl =

Please help with question 2 G-I

Iron oxide reacts with carbon to produce elemental iron and carbon monoxide according the the equation shown below. Consider the reaction of 51.4 grams of Fe2O3 with 24.98 grams of C to produce 19.20 grams of Fe. Fe2O3(s)+3c(s)-------2Fe(s)+3CO(g) a. actual yield b. theoretical yield c. percent yield

Consider the following unbalanced equation. How many molecules of hydrogen will be required to produce 1.60 mol of water?H2 + O2  H2O

Question Completion Status: QUESTION 2 Balancing refers to the number of substances put INTO a reaction has to equal the number of substance PRODUCED by the reaction. This means there must be an understanding of HOW MANY of something is put into a reaction. Match the following description with the HOW MANY X of each substance. Answers may be used once, more than once, or not at all. Example: 6 X3Cl means I have/need 18 X's Example: 10 HX means I have/need 10 X's Etc. - - - - - 3 X20 ✓ 2 Cax 4 XF2 5 AIX3 1 PBX4 ✓2 KX Click Save and Submit to save and submit. Click Save All Answers to save all answers. -4-531 84 A. 2X's B. 5 C. 15 X's D. 3 E. 4 X's F. 10 G. None of these H. 6X's 1.20 3000 103931 401818 / HOTEL hole-he artbl Save All Answers

TRkäM99B-AECYR¡FR6U4K_z_eyCn21R-1ISqFa7wrU1kQTdvvAqYicedUaz64pZZytGhs.. ☆ O CHEMICAL REACTIONS 三 Solving moles-to-moles limiting reactant problems CHLOE 0/5 Nitrogen dioxide (NO,) gas and liquid water (H,O) react to form aqueous nitric acid (HNO,) and nitrogen monoxide (NO)gas. Suppose you have 7.0 mol of NO, and 9.0 mol of H,O in a reactor. Could half the NO, react? O yes 圖 O no If you answered yes, calculate how many moles of HNO, would be produced. Omol Round your answer to the nearest 0.1 mol. Ar Explanation Check 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessibility DII DD 吕0 888 F12 67 FR F9

Liquid hexane (C6H14) burns into oxygen. Overall chemical equation, type of reaction and net ionic equation.